b) elements with different boiling points
c) compounds with identical boiling points
d) compounds with different boiling point
Option-D (Compounds with different boiling point)
Compound is defined as a molecule which is made up of two or more different elements. All compounds are molecules but all molecules are not compounds, for example N₂, O₂, S₈, H₂, F₂ etc are molecules but they are not compounds.
Petroleum is a crude mixture of variety of hydrocarbons containing carbon and hydrogen as a primary elements along with other hetero elements like nitrogen, oxygen and sulfur etc. Therefore, these hydrocarbons can be termed as compounds because they are made up of atleast two essential elements like hydrogen and carbon.
Secondly, the process of distillation works on the basis of difference in boiling points of the compounds present in Petroleum. Therefore, compounds with lower boiling point will evaporate first and will separate first from the mixture and vice versa.
b. hazardous
c. domestic
Answer: Option (b) is the correct answer.
Explanation:
When a substance is used and thrown away which can lead to damage in the environment as it may [produce some toxic or hazardous gases is known as a hazardous waste.
These wastes can be solid, liquid or gaseous.
For example, batteries, kerosene, garden chemicals etc are all hazardous waste.
A domestic waste is a waste thrown by a household which may include paper, vegetable waste, cardboard, yard clippings etc.
Thus, we can conclude that hazardous wastes are solid, liquid, or gas wastes that are toxic, flammable, corrosive, reactive, or radioactive.
endothermic and exothermic reactions.
4
O Endothermic reactions absorb heat
energy while exothermic reactions
release heat energy.
O Exothermic reactions absorb heat
energy while endothermic reactions
release heat energy.
O Endothermic and exothermic reactions
absorb thermal energy.
O Endothermic and exothermic reactions
release thermal energy.
REM
The prefix exo-
applied to a che
mean energy
re
Statement-1 is the correct answer that is Endothermic reactions absorb heat energy while exothermic reactions release heat energy.
How can we distinguish between exothermic and endothermic processes?
Chemical reactions that release energy are referred to as exothermic. More energy is produced than is needed to break the bonds between the reactants when bonds are formed in the byproducts of exothermic processes.
Chemical processes that either use or absorb energy are referred to as endothermic. In endothermic reactions, more energy is absorbed when bonds in the reactants are broken than is released when new bonds are formed in the products. Since an isothermic chemical reaction uses exactly as much energy as it produces, there is no net energy change.
Therefore, the first statement is the right response.
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(1) 6 (2) 8 (3) 16 (4) 32
Answer: it’s 16
Explanation: trust me on this one
The totalpressure in the container is 1.03 atm, which is the sum of the pressure of the carbon dioxide (1 atm) and the partial pressure of the water vapor (0.03 atm) at 25.0°C.
The question is asking about the total pressure in a container after the sublimation of carbon dioxide at a certain temperature in the presence of water. Carbon dioxide sublimates (turns from solid directly to a gas) at normal atmospheric pressure, which is 1 atm. Sublimation is a phase transition in which a solid turns into a gas without passing through the liquid phase. In this case, the CO2 sublimates and is collected in a container over water.
However, as the gas is collected over water, it also becomes saturated with water vapor. The total pressure in the container is therefore the sum of the partial pressure of the carbon dioxide plus the partial pressure of the water vapor. At 25.0°C, the partial pressure of the water vapor is about 0.03 atm. Therefore, the total pressure in the container will be 1 atm (from the CO2) + 0.03 atm (from the water vapor) = 1.03 atm. This is the total pressure in the container.
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The total pressure in the container is 1.03 atmospheres, combining the pressure of sublimated CO2 (1.00 atm) and the vapor pressure of water at 25.0 °C (0.03 atm).
To determine the total pressure in the container containing carbon dioxide and water vapor, we need to consider both the dry gas pressure and the vapor pressure of water. Carbon dioxide sublimes at 1.00 atm at standard atmospheric pressure. However, the gas collected over water becomes saturated with water vapor. The pressure of the pure CO2 gas is therefore equal to the total pressure minus the vapor pressure of the water. The vapor pressure of water at 25.0 °C is approximately 0.03 atm. Therefore, the total pressure in the container is the sum of the pressure due to the carbon dioxide and the water vapor, which equals 1.00 atm + 0.03 atm = 1.03 atm.
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